A mixture containing 3 moles each of C 4 H 8 and C 6 H 6 undergoes complete combustion with O 2 to form CO 2 and H 2 O . Calculate total mass of CO 2 produced

Question

A mixture containing 3 moles each of C 4 ​ H 8 ​ and C 6 ​ H 6 ​ undergoes complete combustion with O 2 ​ to form CO 2 ​ and H 2 ​ O . Calculate total mass of CO 2 ​ produced

TestHub · Accepted Answer

Question Explanation: Calculating the mass of a product in a combustion reaction.

Concept: Stoichiometry and Molar Mass.

Solution: To find the total mass of $CO_{2}$ , write separate balanced combustion equations for each hydrocarbon. Use stoichiometry to find the moles of $CO_{2}$ produced from the given moles of each reactant. Finally, convert the total moles of $CO_{2}$ to mass using its molar mass $(44 g / mol)$ .

$C_{4} H_{8} + C_{6} H_{6} + \frac{27}{2} O_{2} \to 10 C O_{2} + 7 H_{2} O$

$(1 + 1) = 2 m o l$ $10 m o l$ of $C O_{2}$ .

If $(3 + 3) = 6 m o l$ $\frac{10}{2} \times 6 = 30 m o l$

So, the mass of $C O_{2}$ is $30 \times 44 = 1320 g$ .

Final Answer: $1320 g$

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